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- 5-39 An 8.00-g sample of a gas occupies 22.4 L at 2.00 atm and 273 K. What is the molar mass of the gas?5-37 A sample of a gas at 77°C and 1.33 atm occupies a volume of 50.3 L. (a) How many moles of the gas are present? (b) Does your answer depend on knowing what gas it is?Assume the folowing simpifed dependernce of the pressure ina ventricle of the human heart as a function of the volume of blood pumped. 75 150 V(on) • Part A The systale pressure. P.10 mm Hg, comeponding le 1.76x 10' Pa The dastoie prese, Pis 0 mam Hle, comesponding to L11 10 Pa the vome of bd pumped in one heaeat is 75.0 m, calte the work done in a Express your anewer to twe decimal places and include the ppropriate units aunssae
- 3H2(g)+N(g)t>2NH3/g) +Heat owhat is the Keqifthe coscentration atequilibr'um are (H2] =lo01 M: [Nz]= 0.250 M and CNH3]=1.50M? PHow many gramsofnitrogen g as are needect to produce 5OLof ammonia at STP3まらPressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…60°F Cloudy Aktiv Chemistry C KU Portal < https://app.101edu.co D2L E Ch 1 Introduction... Aktiv Chemistry || | || || ||| Connect-Big Google Docs CB Grade Calculator L R Point Grade Calcula... Question 22 of 25 If 70.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? H₂CO3(aq) → H₂O(l) + CO₂(g) Class Search How to St
- (1) + 250 6) ->16 cO2(6) 1842 18 if liquid Octone has a den Sity of 0-70sg/mL how mang moleccules of oxygen gas at STP are Cons umed← O Aktiv Chemistry Esc KU Portal D2 D2L https://app.101edu.co 457 Pantly sunny 1 X + Ch. 1 Introduction -... (@ 2 Aktiv Chemistry A chamber contains equal molar amounts of H2, N2, and O₂. If the total chamber pressure is 2.00 atm, then the partial pressure of H₂ is: #3 Connect-Bio Google Docs F3 $ 4 DII % 5 CG Grade Calculator .... R Point Grade Calcula... FS Question 28 of 30 Q FE A 6 * F7 & 7 PrtScn Class Sear Home 8The concentration of a gas is related to its pressure by the ideal gas law: Concentration (mol) = = = RT where R is the ideal gas constant (0.08314_L-bar :), n is the number of moles, V is volume, P is pressure, and T is mol-K absolute temperature. If the maximum pressure of ozone in the Antarctic stratosphere is 19 mPa and the temperature is -70°C, find the molar concentration of ozone. O 1.126 x 10-10 O 1.126 x 10-8 O 1.126 x 10-5 O 1.126 x 10-3
- P 1) Pinte X A ACTIVITY X EX_FjXNtRGOvhgYzM_rMIZzEwnvfJ17evaEjsK94/edit# Last edit was 2 minutes ago 11 BIUA 田回▼ 1三 ニ=,E▼E ... .. 1. Calculations A. Direction: Calculate the given problems and use the gas laws to determine pressure, volume, or temperature of a gas under certain conditions of change. Show your solutions. Encirce your final answer. 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature. 2. If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature? 3. At 300 K, the given amount of fluorine gas has a volume of 30.0 L. What will be the temperature if the gas occupies a volume of 25 L at constant pressure? 4. A certain gas sample has a volume of 40.00 L at 273 K. At constant pressure. the volume increase to 50 00 L What will be the final temperature of the gas? 5 At…n Unknown elemental metal was reacted with Hydrochloric Acid. It was determined that this reaction evolved Hydrogen gas and left the metal in solution in the 2+ oxidation state. The Unknown metal was then subjected to the same test as Magnesium in the “Molar Mass of Magnesium” lab. After some adjustments to get the volume of gas collected in the right range, the following results were obtained: Mass of Metal used = 0.3682 g P (atmospheric) = 761.1 mm Hg Temperature of gas = 21.6 degrees C Volume of gas collected = 67.5 ml Difference in height of solution levels in the buret and beaker = 163.0mm Vapour pressure of H20 at gas temperature = 19.349 mm Hg Some Constants: R = 0.0820575 L*Atm/mol/K = 62.3637 L*mmHg/mol/K dsolution = 1.00g/ml dHg = 13.6 g/ml From this data, calculate and report the molar mass of the unknown metal with correct significant figures and unit1. A piece of metal "X" weighing 0.0382 g was placed in an eudiometer containing dilute aqueous HCI. After the metal fully dissolved,15.4 mL of hydrogen gas was collected by displacement of water and a 400 mm column of water was observed. The water temperature was 25 degrees Celcius and the barometric pressure was 758.8 mm Hg (torr). Refer to the introduction and data sheet to solve the following problems. a) Calculate the volume occupied by the hydrogen gas at STP. b) How many moles of the metal were consumed in the reaction? c) What is the molar mass of the metal?